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DAT general chemistry formula sheet, Cheat Sheet of Chemistry

Formula equations with atomic and electronic structure, chemical solutions, gases, chemical kinetics and equilibria, thermodynamics and thermochemistry and nuclear reactions.

Typology: Cheat Sheet

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DAT General Chemistry Equation Sheet
Chapter 0: General and Lab Concepts Review
Dilutions
๐‘€1๐‘‰1=๐‘€2๐‘‰2 or
๐ถ1๐‘‰1=๐ถ2๐‘‰2
๐‘€ ๐‘œ๐‘Ÿ ๐ถ= ๐‘ ๐‘œ๐‘›๐‘๐‘’๐‘›๐‘ก๐‘Ÿ๐‘Ž๐‘ก๐‘–๐‘œ๐‘›
๐‘‰=๐‘ฃ๐‘œ๐‘™๐‘ข๐‘š๐‘’
Percent Error
(๐ดโˆ’๐‘‡)
๐‘‡ร—100
๐‘‡=๐‘กโ„Ž๐‘’๐‘œ๐‘Ÿ๐‘’๐‘ก๐‘–๐‘๐‘Ž๐‘™
๐ด=๐‘Ž๐‘๐‘ก๐‘ข๐‘Ž๐‘™
Absorbance
(Spectro-
photometer)
๐ด๐‘๐‘ =๐œ€๐‘๐‘™
๐œ€ =๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ ๐‘’๐‘ฅ๐‘ก๐‘–๐‘›๐‘๐‘ก๐‘–๐‘œ๐‘›
๐‘๐‘œ๐‘’๐‘“๐‘“๐‘–๐‘๐‘–๐‘’๐‘›๐‘ก (๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ
๐‘Ž๐‘๐‘ ๐‘œ๐‘Ÿ๐‘๐‘ก๐‘–๐‘ฃ๐‘–๐‘ก๐‘ฆ)
๐‘=๐‘ ๐‘Ž๐‘š๐‘๐‘™๐‘’โ€ฒ๐‘  ๐‘๐‘œ๐‘›๐‘๐‘’๐‘›๐‘ก๐‘Ÿ๐‘Ž๐‘ก๐‘–๐‘œ๐‘›
๐‘™=๐‘๐‘Ž๐‘กโ„Ž ๐‘™๐‘’๐‘›๐‘”๐‘กโ„Ž
Chapter 2: Atomic and Electronic Structure
Energy of a
photon
๐ธ๐‘โ„Ž๐‘œ๐‘ก๐‘œ๐‘› =โ„Ž๐‘“=โ„Ž๐‘
๐œ†
โ„Ž=๐‘ƒ๐‘™๐‘Ž๐‘›๐‘๐‘˜โ€ฒ๐‘  ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
(6.63ร—10โˆ’34๐ฝโˆ™๐‘ )
๐‘“=๐‘โ„Ž๐‘œ๐‘ก๐‘œ๐‘›โ€ฒ๐‘  ๐‘“๐‘Ÿ๐‘’๐‘ž๐‘ข๐‘’๐‘›๐‘๐‘ฆ
๐‘ =๐‘ ๐‘๐‘’๐‘’๐‘‘ ๐‘œ๐‘“ ๐‘™๐‘–๐‘”โ„Ž๐‘ก
(3.0ร—108๐‘š๐‘ 
โ„)
๐œ†=๐‘โ„Ž๐‘œ๐‘ก๐‘œ๐‘›โ€ฒ๐‘ 
๐‘ค๐‘Ž๐‘ฃ๐‘’๐‘™๐‘’๐‘›๐‘”๐‘กโ„Ž
Absorption/
Emission Line
Spectra
Kinetic Energy
of an electron
(Photoelectric
Effect)
๐œ™ =๐‘ค๐‘œ๐‘Ÿ๐‘˜ ๐‘“๐‘ข๐‘›๐‘๐‘ก๐‘–๐‘œ๐‘›
(๐‘š๐‘–๐‘›๐‘–๐‘š๐‘ข๐‘š ๐‘’๐‘›๐‘’๐‘Ÿ๐‘”๐‘ฆ ๐‘›๐‘’๐‘’๐‘‘๐‘’๐‘‘
๐‘ก๐‘œ ๐‘–๐‘œ๐‘›๐‘–๐‘ง๐‘’ ๐‘’๐‘™๐‘’๐‘๐‘ก๐‘Ÿ๐‘œ๐‘›)
Chapter 7: Chemical Solutions
Molarity
๐‘€=๐‘š๐‘œ๐‘™๐‘’๐‘ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘’
๐ฟ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘–๐‘œ๐‘›
Molality
๐‘š=๐‘š๐‘œ๐‘™๐‘’๐‘ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘’
๐‘˜๐‘”๐‘ ๐‘œ๐‘™๐‘ฃ๐‘’๐‘›๐‘ก
Henryโ€™s
Law
๐‘ƒ๐ด=๐‘˜๐ป[๐ด]
๐‘ƒ๐ด=๐‘๐‘Ž๐‘Ÿ๐‘ก๐‘–๐‘Ž๐‘™ ๐‘๐‘Ÿ๐‘’๐‘ ๐‘ ๐‘ข๐‘Ÿ๐‘’ ๐‘œ๐‘“ ๐‘”๐‘Ž๐‘  ๐ด
๐‘˜๐ป=๐ป๐‘’๐‘›๐‘Ÿ๐‘ฆโ€ฒ๐‘  ๐ฟ๐‘Ž๐‘ค ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
(๐‘ฃ๐‘Ž๐‘Ÿ๐‘–๐‘’๐‘  ๐‘๐‘’๐‘Ÿ ๐‘๐‘Ÿ๐‘œ๐‘๐‘™๐‘’๐‘š)
[A] = conc. of gas A
Freezing
Point
Depression
๐›ฅ๐‘‡๐น=โˆ’๐‘–๐พ๐น๐‘š
๐‘–=๐‘ฃ๐‘Ž๐‘›โ€ฒ๐‘ก ๐ป๐‘œ๐‘“๐‘“ ๐‘“๐‘Ž๐‘๐‘ก๐‘œ๐‘Ÿ
๐พ๐น= ๐น. ๐‘ƒ. ๐‘‘๐‘’๐‘๐‘Ÿ๐‘’๐‘ ๐‘ ๐‘–๐‘œ๐‘› ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
๐‘š=๐‘š๐‘œ๐‘™๐‘Ž๐‘™๐‘–๐‘ก๐‘ฆ
Boiling
Point
Elevation
๐›ฅ๐‘‡๐ต=๐‘–๐พ๐ต๐‘š
๐‘–=๐‘ฃ๐‘Ž๐‘›โ€ฒ๐‘ก ๐ป๐‘œ๐‘“๐‘“ ๐‘“๐‘Ž๐‘๐‘ก๐‘œ๐‘Ÿ
๐พ๐ต= ๐ต. ๐‘ƒ.๐‘‘ ๐‘’๐‘๐‘Ÿ๐‘’๐‘ ๐‘ ๐‘–๐‘œ๐‘› ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
๐‘š=๐‘š๐‘œ๐‘™๐‘Ž๐‘™๐‘–๐‘ก๐‘ฆ
Vapor
Pressure
Depression
(Raoultโ€™s
Law)
๐‘ƒ๐‘ ๐‘œ๐‘™๐‘› =๐œ’๐‘ ๐‘œ๐‘™๐‘ฃ๐‘ƒ๐‘ ๐‘œ๐‘™๐‘ฃ0
๐‘ƒ๐‘ ๐‘œ๐‘™๐‘› = ๐‘‰๐‘ƒ ๐‘œ๐‘“ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘–๐‘œ๐‘›
๐œ’๐‘ ๐‘œ๐‘™๐‘ฃ = ๐‘š๐‘œ๐‘™ ๐‘“๐‘Ÿ๐‘Ž๐‘๐‘ก ๐‘œ๐‘“ ๐‘ ๐‘œ๐‘™๐‘ฃ๐‘’๐‘›๐‘ก
๐‘ƒ๐‘ ๐‘œ๐‘™๐‘ฃ0= ๐‘‰๐‘ƒ ๐‘œ๐‘“ ๐‘๐‘ข๐‘Ÿ๐‘’ ๐‘ ๐‘œ๐‘™๐‘ฃ๐‘’๐‘›๐‘ก
Osmotic
Pressure
(๐…)
๐œ‹=๐‘–๐‘€๐‘…๐‘‡
๐‘€ =๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ๐‘–๐‘ก๐‘ฆ ๐‘œ๐‘“ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘’
๐‘–=๐‘ฃ๐‘Ž๐‘›โ€ฒ๐‘ก ๐ป๐‘œ๐‘“๐‘“ ๐‘“๐‘Ž๐‘๐‘ก๐‘œ๐‘Ÿ
๐‘… = 0 .0821 ๐ฟโ‹…๐‘Ž๐‘ก๐‘š
๐‘š๐‘œ๐‘™โ‹…๐พ
๐‘‡=๐‘ก๐‘’๐‘š๐‘.๐‘–๐‘› ๐พ๐‘’๐‘™๐‘ฃ๐‘–๐‘›
Chapter 5: Gases
Pressure
๐‘ƒ=๐น
๐ด
๐น=๐‘“๐‘œ๐‘Ÿ๐‘๐‘’
๐ด=๐‘Ž๐‘Ÿ๐‘’๐‘Ž
Average Kinetic
Energy
๐พ๐ธ๐‘Ž๐‘ฃ๐‘” = 32
โ„๐‘…๐‘‡
๐‘…=8.314 ๐ฝ
๐‘š๐‘œ๐‘™โˆ™๐พ
Root-Mean-
Square Speed
(๐’—)
๐‘ฃ = โˆš3๐‘…๐‘‡
๐‘€๐‘š
๐‘…=8.314 ๐ฝ
๐‘š๐‘œ๐‘™โˆ™๐พ
๐‘€๐‘š= ๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ ๐‘š๐‘Ž๐‘ ๐‘ 
Ideal Gas Law
๐‘ƒ๐‘‰=๐‘›๐‘…๐‘‡
๐‘› =# ๐‘œ๐‘“ ๐‘š๐‘œ๐‘™๐‘’๐‘ 
๐‘… =0.0821 ๐ฟโ‹…๐‘Ž๐‘ก๐‘š
๐‘š๐‘œ๐‘™โ‹…๐พ
Boyleโ€™s Law
๐‘‰โˆ1
๐‘ƒ
Charlesโ€™ Law
๐‘‰โˆ๐‘‡
Avogadroโ€™s Law
๐‘‰โˆ๐‘›
Combined Gas
Law
๐‘ƒ1๐‘‰1
๐‘›1๐‘‡1=๐‘ƒ2๐‘‰2
๐‘›2๐‘‡2
Standard Temp.
& Pressure (STP)
P=1 atm
T=273 K
*1 mol of gas = 22.4 L
at STP
Standard
Conditions
All aqueous species @ 1M
All gaseous species @1 atm
T=298 K
Density
๐‘ƒ(๐‘€๐‘€)
๐‘…๐‘‡ =๐‘š
๐‘ฃ
๐‘€๐‘€=๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ ๐‘š๐‘Ž๐‘ ๐‘ 
๐‘… =0.0821 ๐ฟโ‹…๐‘Ž๐‘ก๐‘š
๐‘š๐‘œ๐‘™โ‹…๐พ
๐‘š=๐‘š๐‘Ž๐‘ ๐‘ 
๐‘ฃ=๐‘ฃ๐‘œ๐‘™๐‘ข๐‘š๐‘’
Daltonโ€™s Law of
Partial Pressures
๐‘ƒ๐‘ก๐‘œ๐‘ก๐‘Ž๐‘™ =๐‘ƒ๐ด+๐‘ƒ๐ต+โ‹ฏ
Daltonโ€™s Law of
Partial Pressures
๐‘ƒ๐ด=๐œ’๐ด๐‘ƒ๐‘ก๐‘œ๐‘ก๐‘Ž๐‘™
๐œ’๐ด= ๐‘š๐‘œ๐‘™ ๐‘“๐‘Ÿ๐‘Ž๐‘๐‘ก๐‘–๐‘œ๐‘›
๐‘œ๐‘“ ๐‘”๐‘Ž๐‘  ๐ด
Grahamโ€™s Law of
Effusion
๐‘Ÿ1
๐‘Ÿ2=โˆš๐‘€๐‘š2
๐‘€๐‘š1
๐‘Ÿ =๐‘Ÿ๐‘Ž๐‘ก๐‘’ ๐‘œ๐‘“ ๐‘’๐‘“๐‘“๐‘ข๐‘ ๐‘–๐‘œ๐‘›
๐‘€ =๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ ๐‘š๐‘Ž๐‘ ๐‘ 
Real Gas
Equation
(๐‘ƒ+๐‘Ž๐‘›2
๐‘‰2)(๐‘‰
โˆ’๐‘›๐‘)=๐‘›๐‘…๐‘‡
๐‘Ž & ๐‘ =๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก๐‘ 
๐‘ ๐‘๐‘’๐‘๐‘–๐‘“๐‘–๐‘ ๐‘ก๐‘œ ๐‘’๐‘Ž๐‘โ„Ž ๐‘”๐‘Ž๐‘ 
๐‘Ž๐‘›2
๐‘‰2 ๐‘๐‘œ๐‘Ÿ๐‘Ÿ๐‘’๐‘๐‘ก๐‘  ๐‘“๐‘œ๐‘Ÿ
๐ผ๐‘€๐น๐‘ 
โˆ’๐‘›๐‘ ๐‘๐‘œ๐‘Ÿ๐‘Ÿ๐‘’๐‘๐‘ก๐‘  ๐‘“๐‘œ๐‘Ÿ
๐‘ฃ๐‘œ๐‘™๐‘ข๐‘š๐‘’
Chapter 8: Chemical Kinetics
General
Rate Law
A + B โ†’ C + D
๐‘Ÿ๐‘Ž๐‘ก๐‘’=๐‘˜[๐ด]๐‘š[๐ต]๐‘›
๐‘˜ =๐‘Ÿ๐‘Ž๐‘ก๐‘’ ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
๐‘š & ๐‘› =๐‘‘๐‘’๐‘ก๐‘’๐‘Ÿ๐‘š๐‘–๐‘›๐‘’๐‘‘
e๐‘ฅ๐‘๐‘’๐‘Ÿ๐‘–๐‘š๐‘’๐‘›๐‘ก๐‘Ž๐‘™๐‘™๐‘ฆ
Rate
Constant
Units
0 ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ = ๐‘€1โˆ™๐‘ โˆ’1
1๐‘ ๐‘ก ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ =๐‘  โˆ’1
2๐‘›๐‘‘ ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜=๐‘€โˆ’1โˆ™๐‘ โˆ’1
3๐‘Ÿ๐‘‘ ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜=๐‘€โˆ’2โˆ™๐‘ โˆ’1
๐‘˜ =๐‘Ÿ๐‘Ž๐‘ก๐‘’ ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
๐‘€=๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ๐‘–๐‘ก๐‘ฆ
s=๐‘ ๐‘’๐‘๐‘œ๐‘›๐‘‘๐‘ 
Arrhenius
Equation
๐‘˜=๐ด๐‘’โˆ’๐ธ๐‘Ž๐‘…๐‘‡
โ„
๐‘˜ =๐‘Ÿ๐‘Ž๐‘ก๐‘’ ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก
๐ด = ๐‘ข๐‘›๐‘–๐‘ž๐‘ข๐‘’ ๐‘ก๐‘œ ๐‘’๐‘Ž๐‘โ„Ž ๐‘Ÿ๐‘ฅ๐‘›
๐ธ๐‘Ž=๐‘Ž๐‘๐‘ก.๐‘’๐‘›๐‘’๐‘Ÿ๐‘”๐‘ฆ
๐‘…=8.314 ๐ฝ
๐‘š๐‘œ๐‘™โˆ™๐พ
๐‘‡=๐‘ก๐‘’๐‘š๐‘.๐‘–๐‘› ๐พ๐‘’๐‘™๐‘ฃ๐‘–๐‘›
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DAT General Chemistry Equation Sheet

Chapter 0: General and Lab Concepts Review

Dilutions ๐‘€ 1 ๐‘‰ 1 = ๐‘€ 2 ๐‘‰ 2 or

Percent Error (๐ด^ โˆ’^ ๐‘‡)

ร— 100

Absorbance

(Spectro-

photometer)

๐ด๐‘๐‘  = ๐œ€๐‘๐‘™ ๐œ€^ =^ ๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ^ ๐‘’๐‘ฅ๐‘ก๐‘–๐‘›๐‘๐‘ก๐‘–๐‘œ๐‘›

Chapter 2: Atomic and Electronic Structure

Energy of a

photon

( 6. 63 ร— 10 โˆ’^34 ๐ฝ โˆ™ ๐‘ )

( 3. 0 ร— 108 ๐‘šโ„^ ๐‘ ^ )

Absorption/

Emission Line

Spectra

Kinetic Energy

of an electron

(Photoelectric

Effect)

๐พ๐ธ๐‘’โˆ’ = ๐ธ๐‘โ„Ž๐‘œ๐‘ก๐‘œ๐‘› โˆ’ ๐œ™ ๐œ™^ =^ ๐‘ค๐‘œ๐‘Ÿ๐‘˜^ ๐‘“๐‘ข๐‘›๐‘๐‘ก๐‘–๐‘œ๐‘›

Chapter 7: Chemical Solutions

Molarity

Molality

Henryโ€™s

Law

๐‘ƒ๐ด = ๐‘˜๐ป [๐ด] ๐‘ƒ๐ด^ =^ ๐‘๐‘Ž๐‘Ÿ๐‘ก๐‘–๐‘Ž๐‘™^ ๐‘๐‘Ÿ๐‘’๐‘ ๐‘ ๐‘ข๐‘Ÿ๐‘’^ ๐‘œ๐‘“^ ๐‘”๐‘Ž๐‘ ^ ๐ด

[A] = conc. of gas A

Freezing

Point

Depression

๐›ฅ๐‘‡๐น = โˆ’๐‘–๐พ๐น ๐‘š ๐‘–^ =^ ๐‘ฃ๐‘Ž๐‘›โ€ฒ๐‘ก^ ๐ป๐‘œ๐‘“๐‘“^ ๐‘“๐‘Ž๐‘๐‘ก๐‘œ๐‘Ÿ

Boiling

Point

Elevation

๐›ฅ๐‘‡๐ต = ๐‘–๐พ๐ต ๐‘š ๐‘–^ =^ ๐‘ฃ๐‘Ž๐‘›โ€ฒ๐‘ก^ ๐ป๐‘œ๐‘“๐‘“^ ๐‘“๐‘Ž๐‘๐‘ก๐‘œ๐‘Ÿ

Vapor

Pressure

Depression

(Raoultโ€™s

Law)

๐‘ƒ๐‘ ๐‘œ๐‘™๐‘› = ๐œ’๐‘ ๐‘œ๐‘™๐‘ฃ ๐‘ƒ๐‘ ๐‘œ๐‘™๐‘ฃ 0 ๐‘ƒ๐‘ ๐‘œ๐‘™๐‘›^ =^ ๐‘‰๐‘ƒ^ ๐‘œ๐‘“^ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘–๐‘œ๐‘›

๐‘ƒ๐‘ ๐‘œ๐‘™๐‘ฃ^0 = ๐‘‰๐‘ƒ ๐‘œ๐‘“ ๐‘๐‘ข๐‘Ÿ๐‘’ ๐‘ ๐‘œ๐‘™๐‘ฃ๐‘’๐‘›๐‘ก

Osmotic

Pressure

๐œ‹ = ๐‘–๐‘€๐‘…๐‘‡ ๐‘€^ =^ ๐‘š๐‘œ๐‘™๐‘Ž๐‘Ÿ๐‘–๐‘ก๐‘ฆ^ ๐‘œ๐‘“^ ๐‘ ๐‘œ๐‘™๐‘ข๐‘ก๐‘’

๐‘… = 0. 0821 ๐ฟ โ‹… ๐‘Ž๐‘ก๐‘š ๐‘š๐‘œ๐‘™ โ‹… ๐พ ๐‘‡ = ๐‘ก๐‘’๐‘š๐‘. ๐‘–๐‘› ๐พ๐‘’๐‘™๐‘ฃ๐‘–๐‘›

Chapter 5: Gases

Pressure

Average Kinetic

Energy

๐พ๐ธ๐‘Ž๐‘ฃ๐‘” = 3 โ„^2 ๐‘…๐‘‡ ๐‘… = 8. 314 ๐ฝ

Root-Mean-

Square Speed

Ideal Gas Law ๐‘ƒ๐‘‰ = ๐‘›๐‘…๐‘‡ ๐‘›^ =^ #^ ๐‘œ๐‘“^ ๐‘š๐‘œ๐‘™๐‘’๐‘ 

Boyleโ€™s Law

Charlesโ€™ Law ๐‘‰ โˆ ๐‘‡

Avogadroโ€™s Law ๐‘‰ โˆ ๐‘›

Combined Gas

Law

Standard Temp.

& Pressure (STP)

P=1 atm

T=273 K

*1 mol of gas = 22.4 L at STP

Standard

Conditions

All aqueous species @ 1M

All gaseous species @1 atm

T=298 K

Density ๐‘ƒ(๐‘€๐‘€)

Daltonโ€™s Law of

Partial Pressures

Daltonโ€™s Law of

Partial Pressures

๐‘ƒ๐ด = ๐œ’๐ด๐‘ƒ๐‘ก๐‘œ๐‘ก๐‘Ž๐‘™ ๐œ’๐ด =^ ๐‘š๐‘œ๐‘™^ ๐‘“๐‘Ÿ๐‘Ž๐‘๐‘ก๐‘–๐‘œ๐‘›

Grahamโ€™s Law of

Effusion

Real Gas

Equation (๐‘ƒ^ +^

๐‘Ž๐‘›^2

๐‘‰^2

๐‘Ž๐‘›^2

๐‘‰^2

Chapter 8: Chemical Kinetics

General

Rate Law

A + B โ†’ C + D

๐‘Ÿ๐‘Ž๐‘ก๐‘’ = ๐‘˜[๐ด]๐‘š[๐ต]๐‘›

e๐‘ฅ๐‘๐‘’๐‘Ÿ๐‘–๐‘š๐‘’๐‘›๐‘ก๐‘Ž๐‘™๐‘™๐‘ฆ

Rate

Constant

Units

0 ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ = ๐‘€^1 โˆ™ ๐‘ โˆ’^1

1 ๐‘ ๐‘ก^ ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ = ๐‘ โˆ’^1

2 ๐‘›๐‘‘^ ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ = ๐‘€โˆ’^1 โˆ™ ๐‘ โˆ’^1

3 ๐‘Ÿ๐‘‘^ ๐‘œ๐‘Ÿ๐‘‘๐‘’๐‘Ÿ: ๐‘˜ = ๐‘€โˆ’^2 โˆ™ ๐‘ โˆ’^1

s= ๐‘ ๐‘’๐‘๐‘œ๐‘›๐‘‘๐‘ 

Arrhenius

Equation

๐‘˜ = ๐ด๐‘’โˆ’๐ธ๐‘Ž^ โ„๐‘…๐‘‡^ ๐‘˜^ =^ ๐‘Ÿ๐‘Ž๐‘ก๐‘’^ ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก

DAT General Chemistry Equation Sheet Chapter 12: Electrochemistry & Redox Reactions

Standard

Cell

Potential

Nernst

Equation

log ๐‘„

t๐‘Ÿ๐‘Ž๐‘›๐‘ ๐‘“๐‘’๐‘Ÿ๐‘Ÿ๐‘’๐‘‘ ๐‘„ = ๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘–๐‘œ๐‘› ๐‘ž๐‘ข๐‘œ๐‘ก๐‘–๐‘’๐‘›๐‘ก

Faradayโ€™s

Law

๐ผ = ๐‘๐‘ข๐‘Ÿ๐‘Ÿ๐‘’๐‘›๐‘ก (Amps) ๐‘ก๐‘  = ๐‘ก๐‘–๐‘š๐‘’ (๐‘ ๐‘’๐‘๐‘œ๐‘›๐‘‘๐‘ ) ๐‘› = # ๐‘œ๐‘“ ๐‘’๐‘™๐‘’๐‘๐‘ก๐‘Ÿ๐‘œ๐‘›๐‘  ๐‘ก๐‘Ÿ๐‘Ž๐‘›๐‘ ๐‘“๐‘’๐‘Ÿ๐‘Ÿ๐‘’๐‘‘ ๐น = ๐น๐‘Ž๐‘Ÿ๐‘Ž๐‘‘๐‘Ž๐‘ฆโ€ฒ๐‘  ๐‘๐‘œ๐‘›๐‘ ๐‘ก๐‘Ž๐‘›๐‘ก ( 96485

๐‘š๐‘œ๐‘™ ๐‘’โˆ’^ )

Chapter 9: Chemical Equilibria

Equilibrium

Constant

Expressions

๐พ๐‘ = [[๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘Ž๐‘›๐‘ก๐‘ ๐‘๐‘Ÿ๐‘œ๐‘‘๐‘ข๐‘๐‘ก๐‘ ]]

๐‘ƒ๐‘๐‘Ÿ๐‘œ๐‘‘๐‘ข๐‘๐‘ก๐‘  ๐‘ƒ๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘Ž๐‘›๐‘ก๐‘ 

Reaction

Quotient (Q)

[๐‘๐‘Ÿ๐‘œ๐‘‘๐‘ข๐‘๐‘ก๐‘ ]

[๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘Ž๐‘›๐‘ก๐‘ ]

Solubility

Product

Constant ( ๐‘ฒ๐’”๐’‘)

[๐‘๐‘Ÿ๐‘œ๐‘‘๐‘ข๐‘๐‘ก๐‘ ]

[๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘Ž๐‘›๐‘ก๐‘ ]

Chapter 10: Acid-Base Equilbria & Titrations

Ionization

Constant

of Water

๐พ๐‘ค = [๐ป 3 ๐‘‚+][ ๐‘‚๐ปโˆ’] = 1 ร— 10 โˆ’^14

@ 25 ยฐC

pH & pOH ๐‘๐ป = โˆ’log[๐ป+]

๐‘๐‘‚๐ป = โˆ’log[๐‘‚๐ปโˆ’]

[๐ป+]

[๐‘‚๐ปโˆ’]

[H+] &

[OH-]

[๐ป+] = 10 โˆ’๐‘๐ป

[๐‘‚๐ปโˆ’] = 10 โˆ’๐‘๐ป

[๐ป+][๐‘‚๐ปโˆ’] = 1 โˆ— 10 โˆ’^14

Weak

Acids

๐ป๐ด + ๐ป 2 ๐‘‚ โ‡Œ ๐ป 3 ๐‘‚+^ + ๐ดโˆ’

[๐ป 3 ๐‘‚+][๐ดโˆ’]

[๐ป๐ด]

[๐ป+] = โˆš๐พ๐‘Ž[๐ป๐ด]

Weak

Bases

๐ดโˆ’^ + ๐ป 2 ๐‘‚ โ‡Œ ๐ป๐ด + ๐‘‚๐ปโˆ’

[๐‘‚๐ปโˆ’][๐ป๐ด]

[๐ดโˆ’]

[๐‘‚๐ปโˆ’] = โˆš๐พ๐‘ [๐ดโˆ’]

pKa & pKb ๐‘๐พ๐‘Ž = โˆ’log[๐พ๐‘Ž]

๐‘๐พ๐‘ = โˆ’log[๐พ๐‘]

๐พ๐‘ค = ๐พ๐‘Ž ร— ๐พ๐‘ = 1

โˆ— 10 โˆ’^14

Larger ๐พ๐‘Ž = smaller p๐พ๐‘Ž =stronger acid Larger ๐พ๐‘ = smaller p๐พ๐‘ =stronger base Neutralization

Reaction

๐‘›๐ด๐‘€๐ด๐‘‰๐ด = ๐‘›๐ต ๐‘€๐ต ๐‘‰๐ต ๐‘›๐ด =^ #^ ๐‘œ๐‘“^ ๐‘š๐‘œ๐‘™๐‘’๐‘ ^ ๐ป+

Buffers

๐‘๐ป = ๐‘๐พ๐‘Ž + log

[๐ดโˆ’]

[๐ป๐ด]

[๐ดโˆ’] = ๐‘๐‘œ๐‘›๐‘. ๐‘œ๐‘“ ๐‘๐‘Ž๐‘ ๐‘’

[๐ป๐ด] = ๐‘๐‘œ๐‘›๐‘. ๐‘œ๐‘“ ๐‘Ž๐‘๐‘–๐‘‘

Chapter 13: Nuclear Reactions

Kinetics

(always 1st

order)

๐‘ = ๐‘ 0 ๐‘’โˆ’๐‘˜๐‘ก ln ๐‘ = ln ๐‘ 0 โˆ’ ๐‘˜๐‘ก ๐‘ก 1 / 2 =

  1. 693 ๐‘˜

*note that ๐‘ก 1 / 2 is independent of concn for 1st^ order rxns

Nuclear

Binding

Energy

๐ธ = ๐›ฅ๐‘š๐‘^2 ๐‘š^ =^ ๐‘š๐‘Ž๐‘ ๐‘ ^ (๐‘€๐‘ˆ๐‘†๐‘‡^ ๐‘๐‘’^ ๐‘–๐‘›^ ๐‘˜๐‘”) ๐‘ = ๐‘ ๐‘๐‘’๐‘’๐‘‘ ๐‘œ๐‘“ ๐‘™๐‘–๐‘”โ„Ž๐‘ก ( 3. 0 ร— 108

Chapter 11: Thermodynamics & Thermochemistry

Enthalpy (H) (๐›ฅ๐ป > 0 ): ๐‘’๐‘›๐‘‘๐‘œ๐‘กโ„Ž๐‘’๐‘Ÿ๐‘š๐‘–๐‘

Enthalpy of

Formation

First Law of

Thermo-

dynamics

๐›ฅ๐ธ = ๐‘ž + ๐‘ค ๐›ฅ๐ธ^ =^ ๐‘โ„Ž๐‘Ž๐‘›๐‘”๐‘’^ ๐‘–๐‘›^ ๐‘–๐‘›๐‘ก๐‘’๐‘Ÿ๐‘›๐‘Ž๐‘™ ๐‘’๐‘›๐‘’๐‘Ÿ๐‘”๐‘ฆ ๐‘ž = โ„Ž๐‘’๐‘Ž๐‘ก ๐‘ค = ๐‘ค๐‘œ๐‘Ÿ๐‘˜

Pressure-

Volume

Work

๐‘ค = โˆ’๐‘ƒ๐›ฅ๐‘‰ ๐‘ƒ^ =^ ๐‘’๐‘ฅ๐‘ก๐‘’๐‘Ÿ๐‘›๐‘Ž๐‘™^ ๐‘๐‘Ÿ๐‘’๐‘ ๐‘ ๐‘ข๐‘Ÿ๐‘’

Calorimetry

Thermal

Energy (q)

๐‘ž = โˆ’๐ถ๐‘๐‘Ž๐‘™๐‘œ๐‘Ÿ๐‘–๐‘š๐‘’๐‘ก๐‘’๐‘Ÿ ๐›ฅ๐‘‡ ๐ถ๐‘๐‘Ž๐‘™๐‘œ๐‘Ÿ๐‘–๐‘š๐‘’๐‘ก๐‘’๐‘Ÿ =^ ๐‘ ๐‘๐‘’๐‘๐‘–๐‘“๐‘–๐‘^ โ„Ž๐‘’๐‘Ž๐‘ก

Heat Curves

& Thermal

Energy (q)

Entropy (S) ๐›ฅ๐‘† = ฮฃ๐‘›๐‘†๐‘๐‘Ÿ๐‘œ๐‘‘๐‘ข๐‘๐‘ก๐‘  โˆ’ ฮฃ๐‘›๐‘†๐‘Ÿ๐‘’๐‘Ž๐‘๐‘ก๐‘Ž๐‘›๐‘ก๐‘ 

Bond

Dissociation

Energy

Gibbโ€™s Free

Energy ( ๐œŸ๐‘ฎ )

๐›ฅ๐บยฐ = ๐›ฅ๐ปยฐ โˆ’ ๐‘‡๐›ฅ๐‘†ยฐ ๐›ฅ๐บยฐ^ =^ ๐‘ ๐‘ก๐‘Ž๐‘›๐‘‘๐‘Ž๐‘Ÿ๐‘‘^ ๐‘๐‘œ๐‘›๐‘‘๐‘–๐‘ก๐‘–๐‘œ๐‘›๐‘ 

Gibbโ€™s Free

Energy ( ๐œŸ๐‘ฎ )